Determine the empirical formula for a 100.00g sample of a compound having 94.07% sulfur and 5.93% hydrogen

The empirical formula is the simplest expression to represent a chemical compound, which indicates the elements that are present and the minimum proportion in whole numbers that exist between its atoms, that is, the subscripts of chemical formulas are reduced to the most integers. small as possible.

Empirical formula in this case

In this case, you know:

Sulfur (S): 94.07%
Hydrogen (H): 5.93%

Assuming a 100 grams sample, the percentages match the grams in the sample. So you have 94.07 grams of sulfur and 5.93 grams of hydrogen.

Then it is possible to calculate the number of moles of each atom in the molecule, taking into account the corresponding molar mass:

Sulfur (S): [tex]\frac{94.07 g}{32.06\frac{g}{mole} }[/tex]= 2.9342 moles
Hydrogen (H): [tex]\frac{5.93 g}{1\frac{g}{mole} }[/tex]= 5.93 moles

The empirical formula must be expressed using whole number relationships, for this the numbers of moles are divided by the smallest result of those obtained. In this case:

Sulfur (S): [tex]\frac{2.9342 moles}{2.9342 moles}[/tex]= 1
Hydrogen (H): [tex]\frac{5.93 moles}{2.9342 moles}[/tex]= 2.02 ≅2

Therefore the H: S mole ratio is 2: 1

Finally, the empirical formula is H₁S₂= HS₂.

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